General Chemistry I (CHM1210)

e) pressure; temperature

A phase diagram shows the states of a substance as a function of _________ and __________. a) concentration; temperature b) pressure; volume c) density; pressure d) volume; temperature e) pressure; temperature

e) orbitals with the same principal quantum number

A shell consists of all... a) orbitals with the same quantum numbers b) electrons with the same quantum number c) orbitals with the same I and mi quantum numbers d) electrons with the same magnetic quantum number e) orbitals with the same principal quantum number

d) neither sufficiently precise nor accurate

A student performed three measurements to determine the density of water at 25 C to four significant Figueres. The known density of water at 25 C to three significant figures is 0.997 g/mL. The student obtained the following results. 1=0.9345 g/mL 2=0.9623 g/mL 3=0.9007 g/mL a)sufficiently precise but not accurate b) sufficiently accurate but not precise c) both sufficiently precise and accurate d) neither sufficiently precise nor accurate e) more data is needed to determine accuracy and precision

b) hydrophobic; hydrophilic

A substance that is _________ will be insoluble in water, but a substance that is ___________ will be soluble in water. a) miscible; immiscible b) hydrophobic; hydrophilic c) hydrophilic; hydrophobic d) hydrophobic; immiscible e) hydrophilic; miscible

a) protons

All atoms of a particular element have the same number of... a) protons b) neutrons c) neutrons and electrons d) protons and neutrons e) isotopes

a) 9.29 g/mL

An 84.6419 g antique coin is thought to be gold. When the coin is placed in a graduated cylinder containing 15.53 mL of water, the water level rises to 26.64 mL. Calculate the density of the coin. a) 9.29 g/mL b) 5.45 g/mL c) 9.11 g/mL d) 0.738 g/mL e) 0.108 g/mL

c) C

Approximately 3.4*10^-3 cubic feet (ft3) of salt can be removed from seawater in a desalination plant each day. How many cubic meters is this? (1ft=0.3048 m) a) 3.4*10^3 m^3 b) 0.120 m^3 c) 9.6*10^-5 m^3 d) 0.028 m^3 e) 8.33 m^3

not 4,2,1,3 (1/2 Correct)

Arrange the subshells in order of increasing energy in a multielectron atom. (1=lowest energy, 4=highest energy) n=3, I=2 n=2, I=0 n=3, I=0 n=4, I=1

a) A

Based on the ratio of cations to anions in representations [A] and [I], which compound is potassium iodide (KI)? a) A b) B c) C d) D e) E f) F g) G h) H i) I

i) I

Based on the ratio of cations to anions in representations [A] and [I], which compound is potassium oxide (K2O)? a) A b) B c) C d) D e) E f) F g) G h) H i) I

a) A

Between [A] and [I], which valence shell s electron experiences the stronger attraction to its nucleus? a) A b) I

84.006 g/mol

Calculate the molar mass of sodium bicarbonate (NaHCO3) which is also known as baking soda.

1.505*10^23 molecules

Calculate the number of molecules in 0.25 mol of strychnine, C21H22N2O2.

center Carbon, 2 oxygen on each side, 2 double bonds, 4 nonbonding electrons on each oxygen atom

Carbon dioxide is a greenhouse gas. Which Lewis structure is correct for carbon dioxide?

In the Lewis structure of CO (carbon monoxide) has triple bond between the carbon and the oxygen. Carbon has 2 nonbonding electrons and oxygen has 2 nonbonding electrons and both atoms have octets. Carbon has a negative charge and oxygen has a positive charge.

Describe the Lewis structure for CO. Refer to bonds, nonbonding electrons and formal charges in your description.

NCN^2- has a triple bond between the carbon and one nitrogen. This same nitrogen has 2 nonbonding electrons. The other nitrogen paired to the carbon has a single bond, a 2- charge and 6 nonbonding electrons. NCN^2- is linear.

Describe the Lewis structure for NCN^2-. Refer to bonds, nonbonding electrons, formal charges, and molecular geometry in your description.

NF3 has a single bond connecting each fluorine atom to the nitrogen atom. The nitrogen has 2 nonbonding electrons and each fluorine atom has 6 nonbonding electrons. The molecular geometry is pyramidal.

Describe the Lewis structure for NF3. Refer to bonds, nonbonding electrons, formal charges, and molecular geometry in your description.

b) volatilities

Distillation may be used to separate components in a mixture based on... a) densities b) volatilities c) sizes d) masses e) solubilities

d) yes, Lewis structures show which atoms are bonded together, which allows for bond polarity determination

Does the Lewis structure for a molecule allow you to determine bond polarity? Why or why not? a) no, Lewis structures do not provide enough information about bonding to determine bond polarity b) no, Lewis structure only provide information about bond angles not polarity c) no, only ball and stick models demonstrate bond polarity d) yes, Lewis structures show which atoms are bonded together, which allows for bond polarity determination e) yes, Lewis structures include polarity calculations

e) in the gas phase at 150 C

Equal amounts of water are present under the following conditions. In which case do the water molecules have the highest kinetic energy? a) in the solid phase as 0 C b) as ice at -10 C c) as steam at 100 C d) in the liquid phase at 80 C e) in the gas phase at 150 C

c) dependent on the amount of a substance present

Extensive properties are... a) identical for all substances b) the physical properties of a substance c) dependent on the amount of a substance present d) based on the temperature of a substance e) independent of a substance's phase

c) explain widely observed phenomena based on extensive testing

For a hypothesis to be considered a valid scientific theory, it must... a) never be modified or expanded b) be voted on by the scientific community and accepted by all c) explain widely observed phenomena based on extensive testing d) be impossible to prove wrong by experiment e) summarize experimental data without trying to predict future results

e) 69.723 u

Gallium has two naturally occurring isotopes with the following masses and natural abundances. Calculate the average atomic mass of Ga. Ga69= 68.9256 u 60.108% Ga71= 70.9247 u 39.892% a) 69.925 u b) 70.127 u c) 69.824 u d) 70.000 u e) 69.723 u

b) 5.5*10^-7 m

Green light in the visible portion of the electromagnetic radiation spectrum has wavelengths around 550 nm. Express this wavelength in meters using exponential notation. a) 5.5*10^9 m b) 5.5*10^-7 m c) 5.5*10^-9 m d) 5.5*10^7 m e) 5.5 m

2

How many carbon (C) atoms are there in one molecule of acetic acid, CH3COOH?

18

How many electrons in the monoatomic ion 32S^2-?

maybe 27.5

How many grams of carbon (C) are there in 11.0 g of acetic acid, CH3COOH? Report the correct number of sig figs.

4

How many hydrogen atoms are there in one molecule of acetic acid, CH3COOH?

maybe 0.170

How many moles of acetic acid, CH3COOH, are there in 10.2 g of acetic acid? Report the correct number of sig figs.

2

How many moles of carbon are there in one mole of acetic acid CH3COOH?

4

How many moles of hydrogen are there in one mole of acetic acid, CH3COOH?

16

How many neutrons in the monoatomic ion 32S^2-?

13

How many protons in the isotope, 27Al?

d) 3

How many resonance structures can be drawn for the carbonate ion, CO3^2-? a) 2 b) 4 c) 1 d) 3 e) 0

e) 4

How many total covalent bonds are in the Lewis structure of HCN? a) 2 b) 1 c) 3 d) 0 e) 4

a) 10

How many valence electrons are contained in the Lewis structure of CO? a) 10 b) 9 c) 8 d) 11 e) 14

d) 5*10^6 atoms

If the diameter of a carbon atom is approximately 140 pm, how many carbon atoms lined up side by side would span a pencil lead with a diameter of about 0.7 mm? a) 5*10^1 atoms b) 5*10^3 atoms c) 5*10^5 atoms d) 5*10^6 atoms e) 5*10^9 atoms

c) C

If the following arithmetic operations are carried out, how many significant figures should be reported in the answer? (.600)(1.5366-0.708)/(2.105-1.83)+(4.510/0.752) a) 1 b) 2 c) 3 d) 4 e) 5

a) electron-electron repulsive forces

In VSEPR theory, molecular geometry is determined by... a) electron-electron repulsive forces b) electron-electron attractive forces c) electron-nucleus attractive forces d) electron-proton attractive forces e) proton-proton repulsive forces

London dispersion

Ion-dipole, dipole-dipole, London dispersion, ion-induced dipole, or hydrogen bonding, what are the strongest intermolecular forces between the molecules in representation C?

dipole-dipole

Ion-dipole, dipole-dipole, London dispersion, ion-induced dipole, or hydrogen bonding, what are the strongest intermolecular forces between the molecules in representation E?

hydrogen bonding

Ion-dipole, dipole-dipole, London dispersion, ion-induced dipole, or hydrogen bonding, what are the strongest intermolecular forces between the molecules in representation G?

4=[B], 3=[F], 1=[H], 2=[D]

Order the nuclei from the fewest neutrons to the most neutrons (1=fewest, 4=most)

lithium nitride Li3N

Predict the formula and given name of the ionic compound formed by the lithium and nitrogen.

2=Na 3=K 1=Na^+

Rank the atoms/ions in order size, smallest to largest.

5=H-F 3=H-Br 1=H-H 4=H-Cl 2=H-I

Rank the following bonds in order of increasing polarity (1=least polar, 5=most polar)

NF3=1 NO3^-=2 NCN^2-=3

Rank the molecules in order of increasing bond angle about each central atom (1=smallest bond angle, 3=largest bond angle)

CO=1 CO2=2 CO3^2-=3

Rank the molecules/ions in order of increasing carbon-oxygen bond lengths (1=shortest, 3=longest)

d) (7 days)*(700 km/1 days)*(11.9 L/100 km)=

Select the correct unit conversion set up for the following: a motorist needs to determine how much gasoline they will need on a trip. The traveler anticipates traveling 700 km per day for he 7 days of the trip. The vehicle operates at 11.9 L of fuel for 100 km of travel.

d) metal

Sodium is best described as a... a) transition metal b) noble gas c) nonmetal d) metal e) metalloid

b) the motion of the CO2 molecules in the solid phase is much more restricted than in the gas phase

Solid carbon dioxide (CO2) can undergo sublimation to form gaseous CO2. Which of the following statements is true? a) in the solid phase, CO2 molecules easily slip pas t each other, and there are areas of randomly ordered molecules b) the motion of the CO2 molecules in the solid phase is much more restricted than in the gas phase c) in the gas phase, CO2 molecules are strongly attracted to each other d) CO2 molecules in the solid phase are easily compressed to smaller volumes e) the CO2 molecules decompose to form carbon and oxygen when they enter the gas phase

d) 346 years

The brightest star in the constellation Ursa Minor (the little dipper) is Polaris, which is also known as the North Star because it is the closest to Earth's celestial North Pole. Assuming light travels 2.998*10^8 m in one second, how long does it take light to travel the 3.27*10^15 km distance from Polaris to Earth? a) 5.02 years b) 346 min c) 182 min d) 346 years e) 7.57 days

c) -128.6 F

The lowest recorded air temperature on Earth was recorded on July 21, 1983, to be -89.2 C at the Russian Vostok Station in Antarctica. What is this temperature in degrees farenheit? a) -21.8 F b) -31.8 F c) -128.6 F d) -17.6 F e) 103.0 F

e) N2=N2^++e^- describes a nitrogen molecule forming a +1 cation

Which of the following is NOT true regarding cations and anions? a) the formation of a chlorine anion can be written as Cl+e^-=Cl^- b) an oxygen molecule can lose an electron to form O2^- c) Ca^2+ represents a calcium atom that has lost two electrons d) N^3- represents a nitrogen atom that has gained three electrons e) N2=N2^++e^- describes a nitrogen molecule forming a +1 cation

d) it is flammable

Which of the following is a chemical property of formaldehyde (CH2O)? a) it has a density of 1.09 g/ml b) it dissolves in water c) it is colorless d) it is flammable e) it is gas at room temperature

e) 0.25 kg

Which of the following represents the largest mass? a) 250 ng b) 25 ug c) 2.5 g d) 0.025 kg e) 0.25 kg

b) enantiomers

Which of the following terms best describes the relationship between these two molecules? a) achiral molecules b) enantiomers c) superimposable images d) identical molecules e) conjugated pi systems

a) A

Which of the nine substances has the lowest boiling point? a) A b) B c) C d) D e) E f) F g) G h) H i) I

NF3

Which of these molecules have a permanent dipole? a) NO3^- b) NCN^2- c) NF3

G (for sure) and C

Which processes release energy? a) A b) B c) C d) D e) E f) F g) G h) H i) I

a) A

Which processes require energy? a) A b) B c) C d) D e) E f) F g) G h) H i) I

B, F, G, H

Which pure substances are compounds? a) A b) B c) C d) D e) E f) F g) G h) H i) I

C, D, and I

Which pure substances are elements? a) A b) B c) C d) D e) E f) F g) G h) H i) I

A, B, D, and I

Which representation depicts a quantized process? a) A b) B c) C d) D e) E f) F g) G h) H i) I

a) A

Which representation depicts a solid solution? a) A b) B c) C d) D e) E f) F g) G h) H i) I

d) D

Which representation depicts both covalent bonding and ionic bonding? a) A b) B c) C d) D e) E f) F g) G h) H i) I

c) C

Which representation depicts the gain of an electron? a) A b) B c) C d) D e) E f) F g) G h) H i) I

g) G

Which representation depicts the loss of an electron? a) A b) B c) C d) D e) E f) F g) G h) H i) I

h) H

Which representation depicts the probabilistic nature of quantum mechanics? a) A b) B c) C d) D e) E f) F g) G h) H i) I

F

Which representation is consistent with zero probability of an electron being in the nucleus of an atom? a) A b) B c) C d) D e) E f) F g) G h) H i) I

B, E, F, G, H, I (partially correct)

Which representations depict covalent bonding? a) A b) B c) C d) D e) E f) F g) G h) H i) I

A and E

Which representations depict homogeneous mixtures? a) A b) B c) C d) D e) E f) F g) G h) H i) I

D (for sure) and C

Which representations depict ionic bonding? a) A b) B c) C d) D e) E f) F g) G h) H i) I

B and H

Which representations depict isotopes? a) A b) B c) C d) D e) E f) F g) G h) H i) I

d) a regular, repeating network of hydrogen bonds between water molecules is formed

Which statement best explains why the density of water decreases as it is cooled from 4.0 C to its normal freezing point? a) all substances contract before freezing b) hydrogen bonds in liquid water longer than they are in ice c) water molecules become more rigid as they cool d) a regular, repeating network of hydrogen bonds between water molecules is formed e) water molecules decrease in size as they cool because energy is released

d) hybrid orbitals generally have electron density at angles that minimize electron repulsions and maximize orbital overlap when bonding occurs

Which statement gives the best description of the relationship between hybrid orbitals and molecular shape? a) atomic orbitals on different atoms mix to form hybrid orbitals at angles that minimize bonding b) hybrid orbitals result in bond angles predictions much lower than observed bond angels c) hybridization involves bonding electrons only, because lone pairs of electron will not hybridize d) hybrid orbitals generally have electron density at angles that minimize electron repulsions and maximize orbital overlap when bonding occurs e) atomic orbitals from hybrid orbitals wit regions of electron density at random angles around the nucleus, depending on which atomic orbitals are hybridized

e) ions are held together by shared pairs of electrons

Which statement regarding ionic compounds is FALSE? a) the net charge of an ionic compound is zero b) the energy associated with an ionic bond is a form of electrostatic potential energy c) as the distance between oppositely charged ions decreases, the energy between the two ions decreases until a minimum energy between the ions is reached d) oppositely charged ions arrange themselves to minimize repulsions and maximize attractions e) ions are held together by shared pairs of electrons

[C]

Which would contain more molecules, 100 g of [C] or 100 g of [G]?

[G]

Which would contain more sulfur atoms, 100 g of [C] or 100 g of [G]?

Na^+=1s^2, 2s^2, 2p^6 Na=1s^2, 2s^2, 2p^6, 3s^1 K=1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^1 (mostly correct)

Write the condensed electron configurations for the following atoms/ions: Na^+, Na, K

b) B

What compound contains the most elements? a) A b) B c) C d) D e) E f) F g) G h) H i) I

a) molecular magnetic and optical properties

What does MO theory explain that other bonding theories do not? a) molecular magnetic and optical properties b) molecular shape and polarity c) bond angles d) bonding patterns of atoms e) bonding capacity of atoms

4.84*10^-19 (mostly correct)

What is the change in energy of a hydrogen atom when it undergoes an electronic transition from n initial=(6.00*10^0) to n final=(2.0000*10^0)?

Co2O3

What is the chemical formula of cobalt (iii) oxide?

c) 110.984 u

What is the formula unit mass of calcium chloride (CaCl2)? a) 70.906 u b) 75.531 u c) 110.984 u d) 52.089 u e) 129.839 u

26.98153

What is the mass number for the isotope 27Al?

44.01

What is the mass of the molecule representation [E] in g/mol? Report the correct number of sig figs.

6.5*10^14

What is the minimum frequency of a photon (in Hz) that can eject a photoelectron from Ba metal? (the work function of barium is =4.3*10^-19)

60.052

What is the molar mass of acetic acid, CH3COOH in g/mol? Report the correct number of sig figs.

sulfuric acid and H2SO4

What is the name and formula of the oxoacid formed by oxoanion SO4^2-?

ammonium nitrate

What is the name of the ionic compound NH4NO3?

1: 3d 2: 2s 3: 3s 4: 4p

What is the subshell corresponding to the following sets of quantum numbers? An example of how to write your answer is 2s. n=3, I=2 n=2, I=0 n=3, I=0 n=4, I=1

3.02

What is the wavelength (gamma, in meters) of a radio station operating at a frequency of 99.2 mHz?

b) physical properties

Which characteristics allow chemists to separate mixtures through chromatography, distillation, and filtration? a) energies b) physical properties c) intensive properties d) chemical properties e) extensive properties

a) PCl3

Which compound is capable of dipole-dipole interactions? a) PCl3 b) CS2 c) BF3 d) CF4 e) SF6

d) IF3

Which molecule contains a central atom with an expanded octet? a) N2O b) PF3 c) SeCl2 d) IF3 e) BF3

a) A

Which molecule contains the most atoms? a) A b) B c) C d) D e) E f) F g) G h) H i) I

d) CH2Cl2

Which molecule is polar? a) CO2 b) CF4 c) SiH4 d) CH2Cl2 e) CS2

d) C8H12N4O3

Which of the following compounds contains the most nitrogen atoms per formula unit? a) NH4NO3 b) NaN3 c) N2H4 d) C8H12N4O3 e) (NH4)2SO4

c) C

Which of the following illustrates the law of multiple proportions? a) NO2 always contains one nitrogen atom and two oxygen atoms b) the mass of NO2 is a small whole number multiple of the mass of NO c) the mass ratio of O to N in NO2 is twice that in NO d) NO and NO2 have similar chemical and physical properties e) NO always contains once nitrogen and one oxygen atom